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REDOX REACTIONS EXAM QUESTIONS-IB
CHEMISTRY HL QP L1 SECTION 9 ACTUAL
2026 SITTING EXAM TIPS
1. Aqueous solutions of AgNO3, Cu(NO3)2 and Cr(NO3)3 are
electrolyzed using the same quantity of electricity. How do the
number of moles of metal formed compare?
A. Ag = Cu = Cr
B. Ag > Cu > Cr
C. Ag < Cu < Cr
D. Cu > Ag > Cr
2. The standard electrode potentials for two half-cells involving iron are
given below.
Fe2+(aq) + 2e– → Fe(s) Eο = –0.44 V
Fe3+(aq) + e–→ Fe2+(aq) Eο = +0.77 V
What is the equation and the cell potential for the spontaneous
reaction that occurs when the two half-cells are connected?
A. 3Fe2+(aq) → Fe(s) + 2Fe3+(aq) Eο = +1.21 V
B. Fe2+(aq) + Fe3+(aq) → 2Fe(s) Eο = +0.33 V
C. Fe(s) + 2Fe3+(aq) → 3Fe2+(aq) Eο = +0.33 V
D. Fe(s) + 2Fe3+(aq) → 3Fe2+(aq) Eο = +1.21 V
3. Metallic tin can be produced by the electrolysis of a molten salt
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containing Sn2+ ions. Which change(s) would double the amount
of tin produced?
I. Doubling the current passed
during electrolysis
II. Doubling the time used for
electrolysis
III.
Using Sn4+ ions instead of Sn2+
ions
A. I
only
B. II only
C. I and II only
D. I, II and III
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4. Which of the following factors affect the amount of product formed
during electrolysis?
I. The current used
II. The duration of electrolysis
III. The charge on the ion
A. I and II only
B. I and III only
C. II and III only
D. I, II and III
5. The cyanide ion, CN–, can form two complex ions with iron ions.
The formulas of these ions are [Fe(CN)6]4– and [Fe(CN)6]3–. What is
4– 3–
the oxidation
[Fe(CN)6]number of iron
[Fe(CN)6] in the two complex ions?
–4 –3
+2 +3
+3 +2
A. –3 –4
B.
C.
D.
6. Consider the following reactions.
Cu2+(aq) + 2e– Cu(s) Eο =
+0.34 V Mg2+(aq) + 2e–
Mg(s) Eο = –2.36 V Zn2+(aq) +
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2e– Zn(s) Eο = –0.76 V
Which statement is correct?
A. Cu2+(aq) will oxidize both Mg(s) and Zn(s).
B. Zn(s) will reduce both Cu2+(aq) and Mg2+(aq).
C. Mg2+(aq) will oxidize both Cu(s) and Zn(s).
D. Cu(s) will reduce both Mg2+(aq) and Zn2+(aq).
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REDOX REACTIONS EXAM QUESTIONS-IB
CHEMISTRY HL QP L1 SECTION 9 ACTUAL
2026 SITTING EXAM TIPS
1. Aqueous solutions of AgNO3, Cu(NO3)2 and Cr(NO3)3 are
electrolyzed using the same quantity of electricity. How do the
number of moles of metal formed compare?
A. Ag = Cu = Cr
B. Ag > Cu > Cr
C. Ag < Cu < Cr
D. Cu > Ag > Cr
2. The standard electrode potentials for two half-cells involving iron are
given below.
Fe2+(aq) + 2e– → Fe(s) Eο = –0.44 V
Fe3+(aq) + e–→ Fe2+(aq) Eο = +0.77 V
What is the equation and the cell potential for the spontaneous
reaction that occurs when the two half-cells are connected?
A. 3Fe2+(aq) → Fe(s) + 2Fe3+(aq) Eο = +1.21 V
B. Fe2+(aq) + Fe3+(aq) → 2Fe(s) Eο = +0.33 V
C. Fe(s) + 2Fe3+(aq) → 3Fe2+(aq) Eο = +0.33 V
D. Fe(s) + 2Fe3+(aq) → 3Fe2+(aq) Eο = +1.21 V
3. Metallic tin can be produced by the electrolysis of a molten salt
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containing Sn2+ ions. Which change(s) would double the amount
of tin produced?
I. Doubling the current passed
during electrolysis
II. Doubling the time used for
electrolysis
III.
Using Sn4+ ions instead of Sn2+
ions
A. I
only
B. II only
C. I and II only
D. I, II and III
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4. Which of the following factors affect the amount of product formed
during electrolysis?
I. The current used
II. The duration of electrolysis
III. The charge on the ion
A. I and II only
B. I and III only
C. II and III only
D. I, II and III
5. The cyanide ion, CN–, can form two complex ions with iron ions.
The formulas of these ions are [Fe(CN)6]4– and [Fe(CN)6]3–. What is
4– 3–
the oxidation
[Fe(CN)6]number of iron
[Fe(CN)6] in the two complex ions?
–4 –3
+2 +3
+3 +2
A. –3 –4
B.
C.
D.
6. Consider the following reactions.
Cu2+(aq) + 2e– Cu(s) Eο =
+0.34 V Mg2+(aq) + 2e–
Mg(s) Eο = –2.36 V Zn2+(aq) +
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2e– Zn(s) Eο = –0.76 V
Which statement is correct?
A. Cu2+(aq) will oxidize both Mg(s) and Zn(s).
B. Zn(s) will reduce both Cu2+(aq) and Mg2+(aq).
C. Mg2+(aq) will oxidize both Cu(s) and Zn(s).
D. Cu(s) will reduce both Mg2+(aq) and Zn2+(aq).
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